Help ? Redox titrations Watch

BOBBLE.D.69
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5)Calculate the volume of 0.0200 mol dm-3 potassium manganate (VII) which just reacts with 0.142 g of iron (II) sulphate,
in acid solution.

6) Ammonium iron (II) sulphate crystals have the following formula: (NH4)2SO4.FeSO4.nH2O. In an experiment to find n,
8.492 g of the salt were dissolved and made up to 250 cm3
solution with distilled water and dilute sulphuric acid. A 25.0
cm3
portion of the solution was titrated against 0.0150 mol dm-3 KMnO4, 22.5 cm3
being required. Calculate n.

7) A piece of iron wire weighs 2.225 g. It is dissolved in acid, which oxidises it to Fe2+, and made up to 250 cm3. A 25
cm3
sample required 31.0 cm3
of a 0.0185 mol dm-3 solution of potassium dichromate. Calculate the percentage of iron
in the wire.


8) A 25.0 cm3
aliquot of a solution containing Fe2+ and Fe3+ ions was acidified and titrated against 0.0200 M potassium
manganate (VII) solution, requiring 15.0 cm3
. Zn reduces Fe3+ to Fe2+ and a second aliquot was reduced by zinc and
after filtering off the excess zinc, was titrated with the same potassium manganate solution, requiring 19.0 cm3
.
Calculate the concentrations of the Fe2+ and Fe3+ in the solution.
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Pigster
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I don't want to do your homework.

Have you tried to do it, yet?

Where have you got up to?
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